19) identify the properties listed below as properties of metals (m), or properties of nonmetals (nm).
a) ______ lose electrons c) ______ gain electrons e) ______ malleable, ductile
b) ______ dull, brittle d) ______ good electrical conductors f) ______ are not conductors
20) identify the periodic family or group name of the following. write the group number and name.
a) the most reactive group of nonmetals _______________________
b) this group is unreactive, and only found in pure form in nature. _______________________
c) this group’s name means “basic”. _______________________
d) this group of metals contains groups 3-12. _______________________
e) this group contains the most reactive group of metals. _______________________
f) these elements are found in the second row of the f-block elements. _______________________
g) this class of elements have both metallic and nonmetallic properties. _______________________
section #4: periodic trends
21) explain why atomic radius decreases going across the period left to right on the periodic table.
_____________________________________________________________________________________
_____________________________________________________________________________________
____ 22) choose the best reason that the atomic radius generally increases moving down a group of elements.
a) the nuclear charge increases. c) the number of neutrons increases.
b) a new octet if formed. d) the number of occupied energy levels increases.
23) which of the following atoms is largest: nitrogen, phosphorus, or arsenic? _____________________
24) find phosphorus, sulfur, and chlorine on the periodic table. which of these is the largest atom? _______________
25) which of the following atoms is smallest: nitrogen, oxygen, or fluorine? _______________________
26) write a definition for ionization energy. ___________________________________________________
_____________________________________________________________________________________
27) which atom would it take more energy to remove its first electron, sodium or aluminum? _____________________
28) as you move left to right across a period, the first ionization energies _______________________
29) as you move from the top of a group to the bottom, the first ionization energies _______________________
____ 30) of the choices below, which gives the correct order of ionization energy?
a) cl s al ar si c) s si cl al ar
b) cl s p si al d) cl s al si ar
31) which of these elements have the highest ionization energy? aluminum, silicon, or phosphorus _____________________
32) why is the third ionization energy of magnesium so much greater than the second ionization energy?
_____________________________________________________________________________________
33) which of these elements has the highest ionization energy? tin, arsenic, or sulfur _____________________
34) list the following atoms in order of decreasing electronegativity. cl, k, & zn _______________
35) what is the general trend of electronegativity as you go down the group on the periodic table?
_____________________________________________________________________________________
36) what element is the most electronegative? _______________________
37) do metals tend to have high or low electronegativities? _______________________
38) which of the following is the smallest: a lithium atom, li⁺ ion, or a sodium atom? _____________________
39) which atom or ion will have the larger radius? na⁺ or k⁺ ______, k⁺ or ca²⁺ ______, f⁻ or cl⁻ ______, f or f⁻ ______
40) what is the trend for reactivity for the alkali metal group? _______________________
the halogens group? ______

Question

19) identify the properties listed below as properties of metals (m), or properties of nonmetals (nm).
a) ______ lose electrons 	 c) ______ gain electrons 		 e) ______ malleable, ductile
b) ______ dull, brittle 	 d) ______ good electrical conductors 	 f) ______ are not conductors
20) identify the periodic family or group name of the following. write the group number and name.
a) the most reactive group of nonmetals 		 _______________________
b) this group is unreactive, and only found in pure form in nature. 	 _______________________
c) this group’s name means “basic”. 		 _______________________
d) this group of metals contains groups 3-12. 	 _______________________
e) this group contains the most reactive group of metals. 	 _______________________
f) these elements are found in the second row of the f-block elements. 	 _______________________
g) this class of elements have both metallic and nonmetallic properties. 	 _______________________
section #4: periodic trends
21) explain why atomic radius decreases going across the period left to right on the periodic table.
_____________________________________________________________________________________
_____________________________________________________________________________________
____ 22) choose the best reason that the atomic radius generally increases moving down a group of elements.
	a) the nuclear charge increases. 		 c) the number of neutrons increases.
	b) a new octet if formed. 		 d) the number of occupied energy levels increases.
23) which of the following atoms is largest: nitrogen, phosphorus, or arsenic? _____________________
24) find phosphorus, sulfur, and chlorine on the periodic table. which of these is the largest atom? _______________
25) which of the following atoms is smallest: nitrogen, oxygen, or fluorine? _______________________
26) write a definition for ionization energy. ___________________________________________________
_____________________________________________________________________________________
27) which atom would it take more energy to remove its first electron, sodium or aluminum? _____________________
28) as you move left to right across a period, the first ionization energies _______________________
29) as you move from the top of a group to the bottom, the first ionization energies _______________________
____ 30) of the choices below, which gives the correct order of ionization energy?
	a) cl > s > al > ar > si 		 c) s > si > cl > al > ar
	b) cl > s > p > si > al 		 d) cl > s > al > si > ar
31) which of these elements have the highest ionization energy? aluminum, silicon, or phosphorus _____________________
32) why is the third ionization energy of magnesium so much greater than the second ionization energy?
_____________________________________________________________________________________
33) which of these elements has the highest ionization energy? tin, arsenic, or sulfur _____________________
34) list the following atoms in order of decreasing electronegativity. cl, k, & zn _______________
35) what is the general trend of electronegativity as you go down the group on the periodic table?
_____________________________________________________________________________________
36) what element is the most electronegative? _______________________
37) do metals tend to have high or low electronegativities? _______________________
38) which of the following is the smallest: a lithium atom, li⁺ ion, or a sodium atom? _____________________
39) which atom or ion will have the larger radius? na⁺ or k⁺ ______, k⁺ or ca²⁺ ______, f⁻ or cl⁻ ______, f or f⁻ ______
40) what is the trend for reactivity for the alkali metal group? _______________________
	the halogens group? ______

Accepted Answer

### Question 19 #### a) # Brief Explanations: Metals tend to lose electrons to form cations. # Answer: m #### b) # Brief Explanations: Nonmetals are generally dull and brittle (unlike the shiny, malleable metals). # Answer: nm #### c) # Brief Explanations: Nonmetals tend to gain electrons to achieve a stable electron configuration (like forming anions). # Answer: nm #### d) # Brief Explanations: Metals are good electrical conductors due to their free - moving electrons. # Answer: m #### e) # Brief Explanations: Malleability (ability to be hammered into sheets) and ductility (ability to be drawn into wires) are characteristic properties of metals. # Answer: m #### f) # Brief Explanations: Nonmetals are poor conductors of electricity (insulators or semiconductors in some cases). # Answer: nm ### Question 20 #### a) # Brief Explanations: The halogens (group 17) are the most reactive nonmetals as they need only one electron to complete their octet and are highly electronegative. # Answer: Group 17, Halogens #### b) # Brief Explanations: Noble gases (group 18) have a full valence electron shell, making them unreactive and found in pure form in nature. # Answer: Group 18, Noble Gases #### c) # Brief Explanations: Alkaline earth metals (group 2) - the name "alkaline" is related to their basic (alkaline) nature when reacting with water. # Answer: Group 2, Alkaline Earth Metals #### d) # Brief Explanations: The transition metals are the elements in groups 3 - 12 of the periodic table. # Answer: Groups 3 - 12, Transition Metals #### e) # Brief Explanations: Alkali metals (group 1) are the most reactive metals as they have one valence electron which is easily lost. # Answer: Group 1, Alkali Metals #### f) # Brief Explanations: The second row of the f - block elements is called the Actinides. # Answer: Actinides #### g) # Brief Explanations: Metalloids have properties intermediate between metals and nonmetals, showing both metallic and nonmetallic characteristics. # Answer: Metalloids ### Question 21 # Brief Explanations: As we move from left to right across a period, the number of protons in the nucleus (nuclear charge) increases. The electrons are added to the same principal energy level. The increased positive charge of the nucleus pulls the electrons in the same energy level more strongly, resulting in a decrease in the atomic radius. # Answer: As we move left to right across a period, the nuclear charge increases while electrons are added to the same energy level. The increased nuclear charge pulls the electrons more strongly, reducing the atomic radius. ### Question 22 # Brief Explanations: - Option a: An increase in nuclear charge would tend to pull electrons closer, decreasing the radius, so this is incorrect. - Option b: Formation of an octet is not related to the increase in atomic radius down a group. - Option c: The number of neutrons does not directly affect the atomic radius. - Option d: As we move down a group, each element has one more occupied energy level than the one above it. The outermost electrons are further from the nucleus, so the atomic radius increases. # Answer: d) The number of occupied energy levels increases. ### Question 23 # Brief Explanations: Nitrogen (N), phosphorus (P), and arsenic (As) are in the same group (group 15). As we move down a group, the number of occupied energy levels increases. Arsenic is below phosphorus and nitrogen in the group, so it has more energy levels and a larger atomic radius. # Answer: arsenic ### Question 24 # Brief Explanations: Phosphorus (P), sulfur (S), and chlorine (Cl) are in the same period (period 3). As we move from left to right across a period, the atomic radius decreases due to increasing nuclear charge. Phosphorus is the left - most among them, so it has the largest atomic radius. # Answer: phosphorus ### Question 25 # Brief Explanations: Nitrogen (N), oxygen (O), and fluorine (F) are in the same period (period 2). As we move from left to right across a period, the atomic radius decreases. Fluorine is the right - most among them, so it has the smallest atomic radius. # Answer: fluorine ### Question 26 # Brief Explanations: Ionization energy is the minimum amount of energy required to remove the most loosely held (valence) electron from an atom in its gaseous state. # Answer: Ionization energy is the minimum energy required to remove a valence electron from a gaseous atom. ### Question 27 # Brief Explanations: Sodium (Na) has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{1}$, and aluminum (Al) has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}$. Aluminum has a higher nuclear charge than sodium. Also, the electron to be removed from Al is in a more stable (filled 3s) sub - shell compared to the 3s electron in Na? No, actually, the nuclear charge of Al (13 protons) is higher than that of Na (11 protons). The outermost electron of Al is more strongly attracted to the nucleus. So it takes more energy to remove the first electron from aluminum. # Answer: aluminum ### Question 28 # Brief Explanations: As we move left to right across a period, the nuclear charge increases and the electrons are added to the same energy level. The outermost electrons are held more tightly, so more energy is required to remove them. Thus, the first ionization energies generally increase. # Answer: generally increase ### Question 29 # Brief Explanations: As we move from the top to the bottom of a group, the number of occupied energy levels increases. The outermost electrons are further from the nucleus and are shielded by inner electrons. So less energy is required to remove the outermost electron, and the first ionization energies generally decrease. # Answer: generally decrease ### Question 30 # Brief Explanations: - The general trend of ionization energy across a period (left to right) is that it increases (with some exceptions). - Argon (Ar) is a noble gas with a full valence shell, so it has a very high ionization energy. - Among Cl, S, P, Si, Al: Al < Si < P < S < Cl (with P having a slightly lower ionization energy than S due to electron - electron repulsion in the half - filled p - subshell, but overall the trend holds). Option b: Cl > S > P > Si > Al follows the general trend (and accounts for the P - S exception). - Option a: Ar has a higher ionization energy than Si, so this is wrong. - Option c: Ar has a higher ionization energy than Al, S, Si, Cl, so this is wrong. - Option d: Ar has a higher ionization energy than Si, so this is wrong. # Answer: b) Cl > S > P > Si > Al ### Question 31 # Brief Explanations: Aluminum (Al), silicon (Si), and phosphorus (P) are in the same period (period 3). As we move from left to right across a period, the ionization energy generally increases (due to increasing nuclear charge and decreasing atomic radius). Phosphorus is the right - most among them, so it has the highest ionization energy. # Answer: phosphorus ### Question 32 # Brief Explanations: Magnesium has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{2}$. The first ionization energy is the energy to remove one electron from $3s^{2}$ to form $Mg^{+}$, the second ionization energy is to remove the second electron from $3s^{1}$ to form $Mg^{2+}$. After removing two electrons, $Mg^{2+}$ has a noble gas (neon) electron configuration ($1s^{2}2s^{2}2p^{6}$), which is very stable. Removing a third electron would require breaking into the stable inner electron shell (the 2p sub - shell), which requires a large amount of energy. # Answer: After losing two electrons, Mg²⁺ has a stable noble gas electron configuration. Removing a third electron requires breaking into this stable inner shell, which needs much more energy. ### Question 33 # Brief Explanations: Tin (Sn) is in group 14, period 5; arsenic (As) is in group 15, period 4; sulfur (S) is in group 16, period 3. As we move up a group and right across a period, ionization energy increases. Sulfur is in the highest period (lowest principal quantum number for the outermost electrons) and the right - most group among the three, so it has the highest ionization energy. # Answer: sulfur ### Question 34 # Brief Explanations: Electronegativity generally increases from left to right across a period and decreases from top to bottom in a group. Chlorine (Cl) is in group 17, period 3; zinc (Zn) is in group 12, period 4; potassium (K) is in group 1, period 4. So the order of decreasing electronegativity is Cl > Zn > K. # Answer: Cl > Zn > K ### Question 35 # Brief Explanations: As we go down a group, the number of occupied energy levels increases. The outermost electrons are further from the nucleus and are shielded by inner electrons. So the ability of an atom to attract electrons (electronegativity) decreases. # Answer: Electronegativity generally decreases as we go down a group. ### Question 36 # Brief Explanations: Fluorine has the highest electronegativity among all elements because it has a small atomic radius and a high nuclear charge, which gives it a strong ability to attract electrons. # Answer: Fluorine (F) ### Question 37 # Brief Explanations: Metals tend to lose electrons (they are electropositive), so they have a low ability to attract electrons, meaning they have low electronegativities. # Answer: low ### Question 38 # Brief Explanations: - Lithium atom (Li): has an electron configuration of $1s^{2}2s^{1}$. - $Li^{+}$ ion: has an electron configuration of $1s^{2}$, so it has a smaller radius than the Li atom (loses the 2s electron, and the remaining electrons are pulled closer by the nucleus). - Sodium atom (Na): has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{1}$, which has more energy levels than Li (or $Li^{+}$). But $Li^{+}$ has a smaller radius than Li, and Li has a smaller radius than Na? Wait, no: $Li^{+}$ has a radius smaller than Li (since it has lost an electron and the remaining electrons are in the 1s and 2s? No, $Li^{+}$ is $1s^{2}$, Li is $1s^{2}2s^{1}$. The $Li^{+}$ ion has a smaller radius than the Li atom. Now, compare $Li^{+}$, Li, and Na. The $Li^{+}$ ion has only two electrons in the 1s shell. The Li atom has electrons in 1s and 2s. The Na atom has electrons in 1s, 2s, 2p, and 3s. So the smallest is $Li^{+}$. # Answer: $Li^{+}$ ion ### Question 39 #### $Na^{+}$ or $K^{+}$: # Brief Explanations: $Na^{+}$ has an electron configuration of $1s^{2}2s^{2}2p^{6}$, and $K^{+}$ has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$. $K^{+}$ has more occupied energy levels than $Na^{+}$, so $K^{+}$ has a larger radius. # Answer: $K^{+}$ #### $K^{+}$ or $Ca^{2+}$: # Brief Explanations: $K^{+}$ has 19 protons and 18 electrons, $Ca^{2+}$ has 20 protons and 18 electrons. $Ca^{2+}$ has a higher nuclear charge, so it pulls the electrons more strongly, resulting in a smaller radius. So $K^{+}$ has a larger radius. # Answer: $K^{+}$ #### $F^{-}$ or $Cl^{-}$: # Brief Explanations: $F^{-}$ has an electron configuration of $1s^{2}2s^{2}2p^{6}$, and $Cl^{-}$ has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$. $Cl^{-}$ has more occupied energy levels than $F^{-}$, so $Cl^{-}$ has a larger radius. # Answer: $Cl^{-}$ #### F or $F^{-}$: # Brief Explanations: F atom has 9 protons and 9 electrons, $F^{-}$ has 9 protons and 10 electrons. The extra electron in $F^{-}$ increases electron - electron repulsion, and the same nuclear charge has to pull more electrons, so the radius of $F^{-}$ is larger than that of F. # Answer: $F^{-}$ ### Question 40 #### Alkali metal group: # Brief Explanations: Alkali metals (group 1) have one valence electron. As we move down the group, the atomic radius increases, and the valence electron is further from the nucleus and less tightly held. So the reactivity of alkali metals increases as we move down the group. # Answer: Reactivity increases as we move down the alkali metal group. #### Halogens group: # Brief Explanations: Halogens (group 17) need one electron to complete their octet. As we move down the group, the atomic radius increases, and the nucleus is further from the outermost shell. So the ability to attract an electron (electronegativity) decreases, and reactivity decreases as we move down the halogen group. # Answer: Reactivity decreases as we move down the halogens group.

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Explanation:

Question 19

a)

Answer:

b)